1. Elements, compounds and naming binary ionic compounds Ch.2

2. Organization of the periodic table groups/families –Similar properties periods

3. labels of groups or families

4. Names of groups/families

5. Metals, nonmetals and metalloids

6. Compounds!-combos of elements Diatomics (7) - elements that don’t appear as a single atom in nature –H, N, O, F, Cl, Br, I

7. Two main types of compounds Ionic (m/nm): aka salts…electrons are completely transferred Covalent (nm/nm): aka molecular… electrons are shared

8. Naming compounds- Ionic compounds (metal + nonmetal) Metal= cation (+ charge) Nonmetal=anion (- charge) cation gives electron  anion gets electron

9. Common charges from periodic table Page 64!!!

10. Chemical formulas Charges in ionic compounds = 0 You can predict the chemical formula from charges EX) aluminum and sulfur form a compound

11. Try it Calcium and Bromine Sodium and chlorine Answers CaBr 2 NaCl

12. Naming binary salts (simple ionic compounds) Cation then anion Cation= name of element Anion= root of element and -ide See page 64 for special rules Ex) NaCl and CrI 3 Sodium chloride and chromium (III) iodide

13. Try it SnF 2 Mg 3 N 2 Fe 2 O 3 Cs 2 S Answers Tin (II) Fluoride Magnesium Nitride Iron (III) oxide Cesium sulfide

14. Extra practice 62 and 63

15. homework pg76 #61-64 memorize: name and symbol NCS 1-, C 2 H 3 O 2 1-, MnO 4 1-, NH 4 1+, C 2 O 4 2-, CN 1-, OH 1-, S 2 O 3 2-, S 2 O 8 2 CrO 4 2-, Cr 2 O 7 2-, O 2 1-